To a sample of K3PO4 you add in 1.5 molar equivalents of HCl. 1a. What is...

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To a sample of K3PO4 you add in 1.5 molar equivalents of HCl. 1a. What is...

To a sample of K₃PO₄ you add in 1.5 molar equivalents of HCl.

1a. What is the most likely pH (or pH range) of the resulting sample?

1b. What is the predominant molecular form of the phosphate molecule as a result of adding in the HCl?

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Answer 1

Answer #1

Since you have not mentioned the initial concentration of K3PO4 so I assume that it is a constant value.

1a. The resulting solution will be an acidic so it's pH range must be in between 3-6.

1b. The predominant form will be K2HPO4/KH2PO4.

I hope it helps!!!

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Answer 2

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